Single displacement reactions between different metals and ions can be easily carried out in labs. The results of these experiments can be used to create.

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Presentation transcript:

Single displacement reactions between different metals and ions can be easily carried out in labs. The results of these experiments can be used to create redox tables which allow for prediction of spontaneous reactions. For example when Sn 2+ ions are reacted with Fe a reaction occurs. This happens because Sn 2+ ions have a stronger pull on electrons than Fe atoms. This information can be built into a useful table.

Redox Table IonsMetals If an ion reacts with a metal place the ion higher. If it doesn’t place it lower. Sn 2+ reacts with Fe Sn 2+ Fe Sn 2+ doesn’t react with Cu. Cu Zn 2+ ion does not react with Fe. Zn 2+

IonsMetals Fill in the missing ions and metals. Sn 2+ Fe Cu Zn 2+ Cu 2+ Sn Fe 2+ Zn The strongest oxidizing agents are at the top of the ions column and the strongest reducing agents are at the bottom of the metals column. SOA SRA Decreasing strength Decreasing strength

IonsMetals Any ion above any metal will steal the metals electrons and the reaction will be spontaneous. Cu 2+ ions will steal electrons from Sn, Fe, and Zn. Sn 2+ ions will steal e 1- from Fe and Zn. Fe 2+ will react with Zn. Sn 2+ Fe Cu Zn 2+ Cu 2+ Sn Fe 2+ Zn SOA SRA Decreasing strength Decreasing strength

IonsMetals These half reactions can be written as reductions by adding the electrons to the equations. Sn 2+ Fe Cu Zn 2+ Cu 2+ Sn Fe 2+ Zn SOA SRA Decreasing strength Decreasing strength + 2e 1-  Try question 9 on page on page 678.

Cl 2 is the most reactive, I 2 is the least reactive SOA SRA Cl 2 (aq) + 2e > 2Cl 1- (aq) I 2 (aq) + 2e > 2I 1- (aq) Br 2 (aq) + 2e > 2Br 1- (aq) #9

10. SOA SRA Co 2+ Zn Mg e > Co Zn e > + 2e > Mg

11. SOA SRA Cd 2+ Be 2H 1+ Cd Ca 2+ CuCu e 1- --> + 2e 1- --> H 2 + 2e 1- --> Be e 1- --> + 2e 1- --> Ca

12. It is empirical since experimental observations can be used to verify it. 13. Br 2 (l) Ag(s) I 2 (s) Cu 2+ Cl 2 (aq) Cl 1- (aq) + 2e 1- --> 2Br 1- (aq) Ag 1+ (aq) + 1e 1- --> + 2e 1- --> 2I 1- (aq) (aq) + 2e 1- --> Cu(s) + 2e 1- --> 2

Use the Extended Redox Table on page 804 to answer questions on page 679.